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Inorg. Chem. 2001, 40, 1606-1613
Structural and Spectroscopic Studies of the Versatile Coordination Chemistry of the Chiral Ligand N,N-Bis(1-propan-2-onyl oxime)-L-methionine N′-Methylamide with NiII and ZnII Dell T. Rosa, Jeanette A. Krause Bauer, and Michael J. Baldwin* Department of Chemistry, University of Cincinnati, P.O. Box 210172, Cincinnati, Ohio 45221-0172 ReceiVed August 22, 2000
The potentially pentadentate, chiral ligand N,N-bis(1-propan-2-onyl oxime)-L-methionine N′-methylamide (LMABO) shows remarkable versatility in its coordination chemistry with Ni(II) and Zn(II). In the crystal structure of the ZnCl2 complex of L-MABO, the ligand coordinates to the metal only through its three nitrogen donor groups (one amine and two oximes), with two chloride anions completing the distorted trigonal bipyramidal coordination sphere. In the NiCl2 complex, the three nitrogen donors and the thioether sulfur coordinate, along with two chlorides. The crystal structure of the Ni(NO3)2 complex contains two independent molecules, one of which coordinates the three nitrogens, the thioether sulfur, and the amide oxygen of L-MABO in addition to one nitrate anion. The second molecule coordinates the three nitrogen donors, the amide oxygen, one nitrate anion, and a methanol molecule. Thus, in only three crystal structures, L-MABO demonstrates its ability to provide N3, N3S, N3O, and N3OS donor sets. The thioether-bound complexes are unusual in that they have a predominantly nitrogen environment with a nickel-thioether bond that is not constrained by surrounding donor groups in a macrocyclic or linear polydentate motif. Comparison of the thioether-coordinated and methanol-coordinated molecules in the Ni(NO3) salt of L-MABO demonstrate the effect of the thioether bond on the relative “hardness” of the nickel. The electronic absorption and circular dichroism spectra of the aqueous solutions of the nickel complexes are interpreted in terms of a “descent in symmetry” model based on successive C3V and Cs distortions from octahedral geometry. These ligand field spectra indicate that in aqueous solution all ligand groups except for the three nitrogens of L-MABO are displaced by water. In acetonitrile, the non-nitrogen donors in the nitrate salt may also be displaced, while the chlorides remain coordinated.
Introduction synthesized1
We have recently designed and a series of ligands with mixtures of oxime and amide donor groups in a tripodal amine framework that are designed to stabilize the higher oxidation states of nickel, Ni(III) and Ni(IV), and perhaps promote reactions of the Ni(II) complexes with oxygen upon deprotonation of the ligand. Amidates are well-known to stabilize high oxidation state metal complexes, including Ni(III)2,3 and rarely Ni(IV).4 Oximates also stabilize higher oxidation states of nickel, often preferring Ni(IV) with respect to disproportionation of Ni(III). 5,6 Additionally, oximes may be considered to be reasonable models for the biologically important imidazole donor group of the amino acid histidine. Like other groups used to model histidine, such as pyridyl or pyrazole, the oxime nitrogen has the same sp2 hybridization as imidazole. However, unlike pyridyl, or the pyrazole groups in polydentate ligands connected through one of the nitrogens, the oximes may be deprotonated at a position other than the coordinating atom, similar to histidine. * Author to whom correspondence should be addressed. Fax: (513) 5569239. E-mail:
[email protected]. (1) Goldcamp, M. J.; Rosa, D. T.; Landers, N. A.; Mandel, S. M.; Krause Bauer, J. A.; Baldwin, M. J. Synthesis 2000, 2033-2038. (2) Kimura, E.; Machida, R.; Kodama, M. J. Am. Chem. Soc. 1984, 106, 5497-5505. (3) Collins, T. J.; Nichols, T. R.; Uffelman, E. S. J. Am. Chem. Soc. 1991, 113, 4708-4709. (4) Patra, A. K.; Mukherjee, R. Inorg. Chem. 1999, 38, 1388-1393. (5) Mohanty, J. G.; Singh, R. P.; Chakravorty, A. Inorg. Chem. 1975, 14, 2178-2183. (6) Singh, A. N.; Chakravorty, A. Inorg. Chem. 1980, 19, 969-971.
Incorporation of additional biologically relevant donor groups into these ligands is achieved by using natural amino acids as starting materials.1 This provides a potential fifth donor group as well as a chiral center that allows the use of circular dichroism as an additional spectroscopic tool. In the complexes that are the subject of this paper, L-methionine is used as the starting material resulting in the potentially pentadentate, chiral ligand N,N-bis(1-propan-2-onyl oxime)-L-methionine N′-methylamide (L-MABO, for L-methionine amide bis oxime), with two oximes,
an amide, a tertiary amine, and a thioether available for coordination. As anticipated on the basis of the ability of oximates to stabilize higher oxidation states of nickel, deprotonation of the oxime groups results in reaction of the Ni(II) complexes of L-MABO with O2.7,8 Formation of a stable Ni(III) (7) Rosa, D. T.; Goldcamp, M. J.; Mandel, S.; Krause Bauer, J. A.; Baldwin, M. J. Abstracts of Papers, 220th National Meeting of the American Chemical Society, Washington, DC, August 2000; American Chemical Society: Washington, DC, 2000; Abstract 120. (8) Goldcamp, M. J.; Rosa, D. T.; Landers, N.; Krause-Bauer, J. A.; Baldwin, M. J. Abstracts of Papers, 220th National Meeting of the American Chemical Society, Washington, DC, August 2000; American Chemical Society: Washington, DC, 2000; Abstract 118.
10.1021/ic000971f CCC: $20.00 © 2001 American Chemical Society Published on Web 03/01/2001
The Versatile Coordination Chemistry of L-MABO complex in these reactions has been demonstrated by EPR spectroscopy.9 To sort out the mechanism of the oxygen reactions of this and related Ni(II) complexes, it is first necessary to determine the structures of the starting complexes prior to deprotonation and oxidation. Here, we describe the structures and spectroscopy of several Ni(II) and Zn(II) complexes of the neutral L-MABO ligand. In these chiral complexes, L-MABO acts as a tri-, tetra-, or pentadentate ligand providing N3, N3S, N3O, and N3OS donor sets. Combinations of nitrogen and sulfur donors are common to a number of known nickel metalloenzymes, including the recently discovered Ni-dependent superoxide dismutase,10 the R subunit of CO dehydrogenase,11 and 2-mercaptoethanolinhibited urease.12 The F430 cofactor of methyl-coenzyme M reductase has nickel in an N4-donating corphin that allows axial coordination.13 Although a mechanism in which the methyl thioether sulfur of methyl-coenzyme M coordinates to the nickel is considered unlikely, an inactive form of the enzyme has been shown to have the thiol sulfur of coenzyme M coordinated to the nickel,14 and an intermediate involving coordination of the coenzyme B sulfur has recently been proposed.15 Often, structural information about the coordination environment of the active site metal in metalloenzymes is determined by EXAFS (extended X-ray absorption fine structure) spectroscopy, and an appropriate variety of structurally characterized model complexes is needed for calibration of this method. The importance of appropriate models has been demonstrated by Penner-Hahn and co-workers16 in thorough studies of the parameters necessary for accurate interpretation of the EXAFS of Zn metalloenzymes with mixed N/S environments. The Ni(II) structures reported here are unusual in that they provide a mixed N/O and thioether coordination environment with a “branched” polydentate ligand rather than the macrocyclic or “linear” polydentate ligands in which the thioether coordination is constrained by the surrounding donor groups. The chirality of the complexes permits more detailed exploration of the electronic structure through circular dichroism (CD) spectroscopy. The solution structures of the nickel complexes are addressed by analysis of the ligand field spectra using Gaussian fits of the absorption and CD data. The large differences in the donor ability of the various coordinating groups of the ligand produce energy splittings between the absorption and CD bands within the different ligand field transition manifolds. These data provide an excellent example of the utility of successive descents in symmetry from an idealized octahedral geometry in the interpretation of the ligand field spectra. Experimental Section Materials. Acetonitrile was obtained from Fisher Scientific and stirred over anhydrous Cu2SO4 to remove any amines, dried over (9) Rosa, D. T.; Baldwin, M. J. Unpublished results. (10) Choudhury, S. B.; Lee, J.-W.; Davidson, G.; Yim, Y.-I.; Bose, K.; Sharma, M. L.; Kang, S.-O.; Cabelli, D. E.; Maroney, M. J. Biochemistry 1999, 38, 3744-3752. (11) Xia, J.; Dong, J.; Wang, S.; Scott, R. A.; Lindahl, P. A. J. Am. Chem. Soc. 1995, 117, 7065-7070. (12) Wang, S.; Lee, M. H.; Hausinger, R. P.; Clark, P. A.; Wilcox, D. E.; Scott, R. A. Inorg. Chem. 1994, 33, 1589-1593. (13) Hausinger, R. P. Biochemistry of Nickel; Plenum Press: New York, 1993. (14) Ermler, U.; Grabarse, W.; Shima, S.; Goulbeaud, M.; Thauer, R. K. Science 1997, 278, 1457-1462. (15) Signor, L.; Knuppe, C.; Hug, R.; Schweizer, B.; Pfaltz, A.; Jaun, B. Chem.sEur. J. 2000, 6, 3508-3516. (16) Clark-Baldwin, K.; Tierney, D. L.; Govindaswamy, N.; Gruff, E. S.; Kim, C.; Berg, J.; Koch, S. A.; Penner-Hahn, J. E. J. Am. Chem. Soc. 1998, 120, 8401-8409.
Inorganic Chemistry, Vol. 40, No. 7, 2001 1607 calcium hydride, and distilled from P2O5. Water was purified by filtration through a Barnstead/Thermolyne deionizing column and then distilled from a Corning Mega-Pure System MP-3A. N,N-Bis(1-propan2-onyl oxime)-L-methionine N′-methylamide (L-MABO) was prepared as described previously.1 All other chemicals were obtained from commercial sources and used without further purification. Synthesis of Complexes. [Zn(L-MABO)Cl2] (1). A solution of zinc chloride (0.420 g, 3.29 mmol) in 30 mL of methanol was added with stirring to a solution of L-MABO (1.00 g, 3.29 mmol) in 30 mL of methanol. The colorless solution was layered with 150 mL of ethyl acetate and allowed to diffuse. Colorless, needlelike, X-ray quality crystals precipitated within 2 days and were isolated by filtration (yield: 1.14 g, 79%). 1H NMR (DMSO-d6): 10.55 (s, 2H), 7.61 (b, 1H), 3.15 (m, 1H), 3.11 (m, 4H), 2.59 (d, 3H, J ) 4.07 Hz), 2.44 (t, 2H, J ) 7.17 Hz), 2.04 (s, 3H), 1.82 (m, 2H), 1.73 (s, 6H). 13C NMR (DMSO-d6): 172.08, 154.43, 61.72, 54.79, 30.97, 27.44, 25.79, 14.96, 12.48. Anal. Calcd for ZnC12H24N4O3SCl2: C, 32.68; H, 5.45; N, 12.71. Found: C, 32.82; H, 5.19; N, 12.84. [Ni(L-MABO)Cl2] (2). A solution of nickel chloride hexahydrate (0.78 g, 3.29 mmol) in 30 mL of methanol was added with stirring to a solution of L-MABO (1.00 g, 3.29 mmol) in 30 mL of methanol. The blue solution was layered with 150 mL of ethyl acetate and allowed to diffuse. Blue, needlelike, X-ray quality crystals precipitated within a few hours and were isolated the next day by filtration (yield: 1.21 g, 85%). µeff (297 K): 3.2 µB Anal. Calcd for NiC12H24N4O3SCl2: C, 33.20; H, 5.53; N, 12.91. Found: C, 33.43; H, 5.33; N, 12.71. [Ni(L-MABO)(NO3)][NO3]‚1.5CH3OH (3). A solution of nickel nitrate hexahydrate (0.96 g, 3.29 mmol) in 30 mL of methanol was added with stirring to a solution of L-MABO (1.00 g, 3.29 mmol) in 30 mL of methanol. The blue solution was layered with 150 mL of ethyl acetate and allowed to diffuse. Blue, needlelike, X-ray quality crystals precipitated within a few hours and were isolated the next day by filtration (yield: 1.21 g, 67%). µeff (297 K): 3.3 µB Anal. Calcd for NiC12H24N6O9S‚1.5CH3OH: C, 30.30; H, 5.61; N, 15.71. Found: C, 30.62; H, 5.54; N, 15.54. Physical Measurements. Absorption spectra were obtained on a CARY-14 spectrophotometer with a PC interface supplied by OLIS, Inc. Circular dichroism (CD) spectra were recorded on a Jasco J-715 spectropolarimeter with a PC interface and were baseline corrected by subtraction of a spectrum of solvent in the same 1 cm quartz cell. The absorption and CD spectra were fit with the minimum number of Gaussian functions required for a reasonable simulation of the data using a nonlinear algorithm in the GRAMS/32 software package. 1H and 13C NMR spectra were obtained on a Bruker AC-250 instrument and are reported in ppm vs TMS. Quantitative Technologies, Inc. (Whitehouse, NJ), carried out the elemental analyses. Magnetic moments were measured at room temperature (297 K) using a finely ground powder packed in Alfa Aesar 3.24 mm i.d. quartz sample tubes on a Johnson Matthey magnetic susceptibility balance. Conductivity measurements were made using a Yellow Springs Instrument Co. model 31A conductivity bridge with a model 3401 platinum electrode. Solutions were prepared in the same fashion as those used in the spectroscopic experiments, and measurements were made in triplicate. Samples for mid-infrared spectra were dispersed in a KBr pellet, and samples for far-infrared spectra were dispersed in a Nujol mull and spread on a CsI pellet. A BioRad Excalibur spectrometer with a DTGS electrically cooled detector with a KBr extended range beam splitter was used for the mid-IR, and the same platform with a DTGS far-IR detector with a Mylar 6.25 µm beam splitter was used for the far-IR. Raman samples were prepared by finely grinding the crystalline material with Na2SO4 (10 wt %) and packing it into 1 mm i.d. melting point capillary tubes. Samples were spun at 5000 rpm using a Dremel Moto-Tool during data collection. Raman spectra were obtained using a SPEX 1404 0.85 m double spectrometer with a liquid N2 cooled, 13.6 mm back-thinned SPEX CCD chip detector. Raman scattering was excited at 488 nm (∼300 mW at the sample) with a Coherent 10 W Sabre Ar ion laser and collected from 275 to 2000 cm-1 using a Kaiser Optical Systems holographic SuperNotch filter to modulate the Raleigh line. Raman shifts were calibrated against the laser emission at 488.0 nm.
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Table 1. Crystallographic Data and Structure Refinement for 1, 2, and 3 empirical formula fw temp (K) cryst syst space group unit cell dimens a (Å) b (Å) c (Å) R (deg) β (deg) γ (deg) vol (Å3), Z density (calcd) (Mg/m3) abs coeff (mm-1) Flack param final R indices [I > 2σ(I)] R1 wR2 R indices (all data) R1 wR2
1
2
3
ZnC12H24N4O3SCl2 440.68 294(2) orthorhombic P212121
NiC12H24N4O3SCl2 434.02 150(2) hexagonal P65
NiC12H24N5O6S]NO3‚[NiC13H28N5O7S]NO3 1022.35 150(2) monoclinic P21
8.6833(2) 10.4612(2) 21.0386(3) 90 90 90 1911.10(6), 4 1.532 1.691 0.01(1)
12.4125(2) 12.4125(2) 23.0975(8) 90 90 120 3081.87(13), 6 1.403 1.321 -0.02(2)
10.1231(2) 16.5442(6) 13.6701(5) 90 104.446(2) 90 2217.06(12), 2 1.530 1.026 0.02(2)
0.0314 0.0676
0.0472 0.1110
0.0553 0.1301
0.0402 0.0711
0.0645 0.1203
0.0692 0.1373
X-ray Crystallography. General Procedures. A suitable crystal was mounted on the tip of a glass fiber for data collection. Data were collected17 on a Siemens SMART 1K CCD diffractometer (program v5.051, sealed-tube generator, graphite-monochromated Mo KR radiation). The detector was 5 cm from the crystal. A series of data frames measured at 0.3° increments of ω were collected to calculate a unit cell. Data collection frames were measured at 0.3° intervals of ω. The data frames were processed using the program SAINT v5.A06 (Bruker AXS, Madison, WI). The data were corrected for decay, Lorentz, and polarization effects. Semiempirical absorption correction based on the multiscan technique and beam corrections were applied using SADABS.18 Structures were solved by a combination of direct methods using SHELXTL v5.03 and the difference Fourier technique and refined by full-matrix least squares on F2 for the reflections diffracting out to 0.75 Å.19 The molecules each contain a chiral center, and the absolute configuration was determined on the basis of refinement of the Flack parameter and the effect on the overall R-factor. Non-hydrogen atoms were refined with anisotropic displacement parameters. Hydrogen atom isotropic temperature factors were defined as U(C)a ) U(H) where a ) 1.2 for NH, CH, or CH2 hydrogens, and a ) 1.5 for OH or CH3 hydrogens. Hydrogen atoms were either located directly or calculated on the basis of geometric criteria (methyl H atoms were calculated after locating at least one directly) and treated with a riding model. Disordered methyl groups appear in all three complexes; occupancies for the H atoms were set at 0.5. A suitable disorder model for the methanol solvate in complex 3 could not be resolved; thus the solvent contribution was subtracted from the reflection data using the program SQUEEZE.20 The electrons/unit cell from the solvent were applied to the molecular weight, F(000), and density values reported. Elemental analysis suggests at least 1 fully occupied methanol of crystallization. The final difference map in each case was essentially featureless. Crystallographic data are summarized in Table 1. Final atomic coordinates, displacement parameters, bond distances and angles, and H-bonds are provided as Supporting Information. (17) Data were collected through the Ohio Crystallographic Consortium, funded by the Ohio Board of Regents 1995 Investment Fund (CAP075) located at the University of Toledo, Instrumentation Center in A&S, Toledo, OH 43606. (18) Sheldrick, G. M. University of Goettingen, Germany. (19) G. M. Sheldrick, University of Goettingen, Germany, and Bruker AXS, Madison, WI. (20) Spek, A. L. 1992, University of Utrecht, Utrecht, The Netherlands. SQUEEZE is a routine implemented in PLATON-92 that allows solvent contributions to be eliminated from the reflection data.
Results Structure Descriptions. Figure 1 shows the crystal structure of the Zn(II) complex 1. Selected bond distances and angles are given in Table 2. The molecule crystallizes with only a single zinc complex in the asymmetric unit and no solvent of crystallization. The Zn(II) ion coordinates the ligand L-MABO through its two oxime nitrogens and the tertiary amine. The thioether and amide arms extend out into the lattice. The amide hydrogen participates in a rather weak H-bond with Cl(1) from another molecule (N(1)-H(1)‚‚‚Cl(1); N(1)‚‚‚Cl(1), 3.582(3) Å; H(1)‚‚‚Cl(1), 2.82 Å). The remaining coordination sphere is filled by the two chlorine anions giving a structure best described
Figure 1. ORTEP view (50% probability) of the neutral complex [Zn(L-MABO)Cl2] (1). Methylene and methyl hydrogen atoms are omitted for clarity.
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Inorganic Chemistry, Vol. 40, No. 7, 2001 1609
Table 2. Selected Bond Distances (Å) and Angles (deg) of ZnC12H24N4O3SCl2 (1) and NiC12H24N4O3SCl2 (2) 1 Zn-N(2) Zn-N(3) Zn-N(4)
2
Zn-Cl(1) Zn-Cl(2)
2.411(2) amine Ni-N(1) 2.078(2) Ni-N(2) 2.056(2) Ni-N(3) Ni-S 2.3474(7) Ni-Cl(1) 2.2325(7) Ni-Cl(2)
2.213(3) amine 2.028(3) 2.014(3) 2.3676(11) 2.3532(11) 2.4572(11)
N(2)-Zn-N(3) N(3)-Zn-N(4) N(4)-Zn-N(2) N(2)-Zn-Cl(1) N(3)-Zn-Cl(1) N(4)-Zn-Cl(1) N(2)-Zn-Cl(2) N(3)-Zn-Cl(2) N(4)-Zn-Cl(2)
73.65(7) 115.85(8) 73.83(7) 154.75(5) 92.28(6) 94.74(6) 97.75(5) 109.16(6) 128.86(7)
79.61(13) 90.52(14) 79.35(13) 96.78(9) 176.34(10) 89.35(10) 162.58(9) 87.31(10) 89.40(10) 99.97(9) 94.59(10) 174.64(10) 85.45(4) 92.45(4)
N(1)-Ni-N(2) N(2)-Ni-N(3) N(3)-Ni-N(1) N(1)-Ni-Cl(1) N(2)-Ni-Cl(1) N(3)-Ni-Cl(1) N(1)-Ni-Cl(2) N(2)-Ni-Cl(2) N(3)-Ni-Cl(2) N(1)-Ni-S N(2)-Ni-S N(3)-Ni-S Cl(1)-Ni-S Cl(2)-Ni-S
Figure 3. ORTEP views (50% probability) of the complex cations [Ni(L-MABO)(NO3)][NO3] (3a) and [Ni(L-MABO)(NO3)(CH3OH)][NO3] (3b). Methylene and methyl hydrogen atoms are omitted for clarity. Figure 2. ORTEP view (50% probability) of the neutral complex [Ni(L-MABO)Cl2] (2). Methylene and methyl hydrogen atoms are omitted for clarity.
as distorted trigonal bipyramidal with N(4), N(3), and Cl(2) defining the equatorial plane, and N(2) and Cl(1) as axial ligands. The axial chloride [Zn-Cl(1)] has a significantly longer bond length than the equatorial chloride, and the amine in the other axial position [Zn-N(2), 2.411(2) Å] also has a longer bond length than the other coordinated nitrogens (average ZnN(3,4) distance, 2.067 Å). Figure 2 shows the crystal structure of complex 2, which packs in the relatively uncommon space group P65. The asymmetric unit is composed of a single nickel complex. The Ni(II) coordinates to the ligand (L-MABO) through the oxime nitrogens, the amine nitrogen, and the thioether sulfur. Both chloride anions are also coordinated to complete a distorted
octahedral coordination geometry. Selected bond distances and angles are given in Table 2. The chloride trans to the amine nitrogen of the complex, Cl(2), has a significantly longer bond length than Cl(1). The Ni-Cl(2) bond is also longer than the Ni-S bond. The amide arm participates in one classical intermolecular H-bond, (N(4)-H(4)‚‚‚O(3); N(4)‚‚‚O(3), 2.824(4) Å; H(4)‚‚‚O(3), 1.95 Å). The asymmetric unit of 3 is composed of two nickel complexes a and b (Figure 3a,b) with different coordination environments and a disordered 1/2 methanol of solvation. Unlike the chloride complexes above, only one of the nitrate anions is directly coordinated to the nickel ion. It binds opposite the amine nitrogen in each molecule, while the second nitrate remains uncoordinated in the lattice. This additional available coordination site of the complex allows coordination of two of the available non-nitrogen, nonanion ligands (thioether, amide
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Table 3. Selected Bond Distances (Å) and Angles (deg) of NiC12H24N5O6S]NO3‚[NiC13H28N5O7S]NO3 (3) 3a
3b
Ni(1)-N(1) Ni(1)-N(2) Ni(1)-N(3) Ni(1)-S(1) Ni(1)-O(3) Ni(1)-O(4)
2.080(4) amine 2.054(4) 2.011(4) 2.464(1) 2.078(3) amide 2.024(3) nitrate
Ni(2)-N(6) Ni(2)-N(7) Ni(2)-N(8) Ni(2)-O(13) Ni(2)-O(9) Ni(2)-O(10)
2.115(4) amine 2.049(4) 2.028(5) 2.113(4) methanol 2.049(4) amide 2.019(4) nitrate
N(1)-Ni(1)-N(2) N(2)-Ni(1)-N(3) N(3)-Ni(1)-N(1) N(1)-Ni(1)-O(3) N(2)-Ni(1)-O(3) N(3)-Ni(1)-O(3) N(1)-Ni(1)-O(4) N(2)-Ni(1)-O(4) N(3)-Ni(1)-O(4) N(1)-Ni(1)-S(1) N(2)-Ni(1)-S(1) N(3)-Ni(1)-S(1) O(3)-Ni(1)-S(1) O(4)-Ni(1)-S(1)
81.9(2) 93.6(2) 81.1(2) 79.9(2) 90.0(2) 159.9(1) 166.0(2) 86.4(2) 107.4(2) 99.16(12) 176.31(13) 90.07(12) 86.72(10) 92.04(10)
N(6)-Ni(2)-N(7) N(7)-Ni(2)-N(8) N(8)-Ni(2)-N(6) N(6)-Ni(2)-O(9) N(7)-Ni(2)-O(9) N(8)-Ni(2)-O(9) N(6)-Ni(2)-O(10) N(7)-Ni(2)-O(10) N(8)-Ni(2)-O(10) N(6)-Ni(2)-O(13) N(7)-Ni(2)-O(13) N(8)-Ni(2)-O(13) O(9)-Ni(2)-O(13) O(10)-Ni(2)-O(13)
80.8(2) 89.5(2) 82.0(2) 80.3(2) 94.0(2) 161.1(2) 167.3(2) 92.7(2) 109.0(2) 94.2(2) 175.0(2) 89.3(2) 85.5(2) 92.3(2)
oxygen, and/or solvent). In both 3a and 3b the amide is bound to nickel through the carbonyl oxygen. The thioether S(1) is only bound to nickel in complex 3a, while the nickel in 3b coordinates a methanol molecule O(13) in place of the thioether. Selected bond angles and distances are given in Table 3. Weak, nonclassical H-bonding occurs between the methyl group of the unbound thioether arm in 3b and the coordinated NO3- of 3a in addition to one of the NO3- counterions (C(24A)H(24A)‚‚‚O(19); C(24)‚‚‚O(19), 3.507(8) Å; H(24A)‚‚‚O19, 2.78 Å and C(24)-H(24A)‚‚‚N(3); C(24)‚‚‚N(3), 3.403(7) Å, H(24A)‚‚‚N(3), 2.79 Å). Spectroscopic Characterization. Absorption and CD spectra of 10 mM solutions of the Ni(II) complexes taken at approximately 1 h and 24 h after sample preparation were essentially identical. The aqueous and acetonitrile spectra with their Gaussian fits are shown in Figures 4 and 5, and the fit parameters are tabulated in Tables 4 and 5, respectively. The absorption and CD spectra of the zinc complex 1 in both acetonitrile and water are featureless below 33 000 cm-1, as expected for a d10 metal. The absorption spectra of 2 and 3 in both water and acetonitrile show three bands typical of sixcoordinate d8 nickel complexes.21 The absorption and CD spectra of 2 in acetonitrile, however, are markedly different from the others. The aqua color of this solution also differs from the deep blue-purple color of the others. Coulometric measurements were obtained from aqueous and acetonitrile solutions of 2 and 3 for correlation with the interpretation of the solution spectroscopic data described in the Discussion section. In aqueous solution at the same concentration as the spectroscopic studies described above (10 mM), the conductivity of the chloride, 2 (82.7 S cm2 mol-1), is slightly higher than that of the nitrate, 3 (70.0 S cm2 mol-1). This difference is likely due to the difference in the nature of the anion rather than a difference in the number of ions in solution, as the conductivity of NaCl is slightly higher than the conductivity of NaNO3 in water as well. In acetonitrile, however, the values are more than 20-fold higher for 3 (29.1 S cm2 mol-1) than for 2 (1.32 S cm2 mol-1). This is consistent with both chlorides of 2 remaining coordinated in acetonitrile to give a neutral complex while one or both of the nitrates is dissociated, as seen in the crystal structures. Similarly to the spectroscopic (21) Lever, A. B. P. Inorganic Electronic Spectroscopy; Elsevier: Amsterdam, 1984.
Figure 4. Absorption and CD spectroscopy (solid line) with fits (dotted lines) for (A) 2 in H2O and (B) 3 in H2O.
measurements, no differences were observed in the coulometric data collected 1 h after solution preparation compared to data collected after 24 h. IR and Raman vibrational data were collected and are presented in Table S1 of the Supporting Information. The midIR spectra are reminiscent of the free ligand, while bands between 1500 and 1250 cm-1 indicative of nitrate in its different environments in complex 3 are not well resolved. In the farIR, several bands in the energy range characteristic of ν(NiS) and ν(Ni-Cl) are observed for each complex between 300 and 100 cm-1. The position and order of ν(Ni-S) and ν(NiCl) bands has been shown to be dependent on the nature of the other ligands in the coordination sphere of previously described complexes.22 Thus, definitive assignment of these bands is not possible without isotopic substitution studies. Discussion In the complexes reported here, L-MABO acts as a tridentate N3 (1), tetradentate N3S or N3O (2 and 3b, respectively), or pentadentate N3OS ligand (3a) demonstrating the wide range of possible conformations that can be achieved by this ligand. In all four molecules, the three nitrogen donors from the amine and two oxime groups make up one face of a pseudo-octahedron (22) Schlapfer, C. W.; Saito, Y.; Nakamoto, K. Inorg. Chim. Acta 1972, 6, 284-290.
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Inorganic Chemistry, Vol. 40, No. 7, 2001 1611
Figure 5. Absorption and CD spectroscopy (solid line) with fits (dotted lines) for (A) 2 in CH3CN and (B) 3 in CH3CN. Table 4. UV-Vis (λmax/cm-1 (/M-1 cm-1)) and CD (λ(max -1 (∆/M-1 cm-1)) in Water for Complexes 2 and 3
or
min)/cm
2
3
absorption
CD spectra
absorption
CD spectra
31420 (28.4)
31060 (-0.012) 30010 (0.013)
31420 (26.9)
31060 (-0.009) 30010 (0.010)
25610 (18.6) 23400 (4.5) 14830 (32.5)
23110 (0.011) 17350 (0.005)
